Which from the following statements is correct for aqueous solution of \(6 \mathrm{gL}^{-1}\) urea and \(17 \cdot 12 \mathrm{~g} \mathrm{~L}^{-1}\) of sucrose?
[Molar mass of urea \(=60 \mathrm{~g} \mathrm{~mol}^{-1}\)
Molar mass of sucrose \(=342 \mathrm{~g} \mathrm{~mol}^{-1}\) ]

\(\mathrm{M}_{\text {urea }}=\frac{\text { mass of urea in solution }}{\text { molar mass of urea } \times \text { volume of solution (in } L \text { ) }}\)
\(=\frac{\frac{6 \mathrm{~g}}{60 \mathrm{~g} \mathrm{~mol}^{-1}}}{1 \text { Litre }}=0.1 \mathrm{~mol} \mathrm{~L}^{-1}\)
\(\mathrm{M}_{\text {sucrose }}=\frac{\text { mass of sucrose in solution }}{\text { molar mass of sucrose } \times \text { volume of solution (in } L \text { ) }}\)
\(=\frac{\frac{17.12 \mathrm{~g}}{342 \mathrm{~g} \mathrm{~mol}^{-1}}}{1 \mathrm{Litre}^2}=0.05 \mathrm{~mol} \mathrm{~L}^{-1}\)
Urea has higher solute concentration \((0.1 \mathrm{M})\) than sucrose ( 0.05 M ).
Thus, urea solution is hypertonic to sucrose.